Chemistry

Copper and lead had different densities. Sketch a diagram at the particular nature of matter level showing the atoms of a small cross section of copper and lead. Use this diagram to explain why lead is denser than copper.

I couldn't find any pictures or see anywhere in my textbook about the structures of Cu and Lead, so I was wondering how it would look.
But would this be a right answer to the second part of the answer:
Lead is more denser than copper due to the atoms being packed together closer than those in copper.

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  1. I think your explanation is good. Perhaps these images will help. That's all I could find.

    https://www.google.com/search?q=image+cross+section+copper+particle&tbm=isch&imgil=HL-PiOq6PSpFpM%253A%253Bb1KlgfLW3DflMM%253Bhttp%25253A%25252F%25252Fnewsoffice.mit.edu%25252F2011%25252Fmultiscale-materials-1017&source=iu&pf=m&fir=HL-PiOq6PSpFpM%253A%252Cb1KlgfLW3DflMM%252C_&biw=1024&bih=609&usg=__PBbl0DeKKsLo1JCwWOKwa8Mn9u0%3D&ved=0CC0Qyjc&ei=d7iRVZ-IAcy4-AGZyJ-wBA#imgdii=HL-PiOq6PSpFpM%3A%3BHL-PiOq6PSpFpM%3A%3B9FuNRr5QekS8CM%3A&imgrc=HL-PiOq6PSpFpM%3A&usg=__PBbl0DeKKsLo1JCwWOKwa8Mn9u0%3D

    https://www.google.com/search?q=image+lead+metal+cross+section&tbm=isch&imgil=yoVoqqff1jTSxM%253A%253B1vpyGMIb9SCS2M%253Bhttps%25253A%25252F%25252Fen.wikipedia.org%25252Fwiki%25252FEastern_span_replacement_of_the_San_Francisco%25252525E2%2525252580%2525252593Oakland_Bay_Bridge&source=iu&pf=m&fir=yoVoqqff1jTSxM%253A%252C1vpyGMIb9SCS2M%252C_&biw=1024&bih=609&usg=__7aIelX7QNtRR1iJKw2x0zP_cQBk%3D&ved=0CCoQyjc&ei=57mRVZvkOIzh-QH-8IKIAg#imgdii=yoVoqqff1jTSxM%3A%3ByoVoqqff1jTSxM%3A%3BH3UbvYynXNbVuM%3A&imgrc=yoVoqqff1jTSxM%3A&usg=__7aIelX7QNtRR1iJKw2x0zP_cQBk%3D

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  2. Nope: Lead atoms and copper atoms pack about the same, with the exception that lead has a greater atomic radius than copper (.175nm vs .128), which when cubed gives a volume ratio of (.175/.128)^3 or 2.5. The atomic mass of Pb is 207 vs Cu 63, so the ratio of mass to is 207/63= 3.3
    or comparing the mass density of ocupied atomic volme is 3.3/2.5= 1.32

    Now the observed density of lead is about 11.3, and the density of Cu is
    atomsLead/cm^3= density 8.94, or a ratio of 11.3/8.9 = 1.27 WHICH IS ALMOST THE SAME as the density of the atomic volumes. Bottom line: the packing is nearly the same, the differences in density is due to atomic mass and atomic radius.

  3. Then if I sketch a diagram of a cross section of the atoms of both elements, it would look the same. If they look the same then in my explanation should I say, since both diagrams are the same, the only reason that lead is denser than copper is due to the fact that lead has a bigger atomic radius and mass than copper.

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  4. I agree with that.

  5. So if I were to draw the cross section would I just draw it as so-

    Lead Copper

    ooooooo ooooooo
    ooooooo ooooooo
    ooooooo ooooooo
    ooooooo ooooooo

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